At what temperature does 0.019135 moles of ne in a 878.3 ml container exert a pressure of 0.946 atm?

Temperature is 529.164 K

We are given

Number of moles of Ne (n) =  0.019135 moles

Volume (V) = 878.3 mL

Pressure (P) = 0.946 atm

We are required to calculate the temperature;

We can do this using the ideal gas law equation which is;

PV = nRT, where P is the pressure, n is the number of moles, V is the volume, R is the ideal gas constant (0.082057 Latm/mol/K) and T is the temperature.

From the equation;

Therefore, the temperature will be 529.164 K.

Temperature of gas Ne : 529.208 K

Some of the laws regarding gas, can apply to ideal gas (volume expansion does not occur when the gas is heated), among others  

So that the three laws can be combined into a single gas equation, the ideal gas equation  

In general, the gas equation can be written  

where  

P = pressure, atm  

V = volume, liter  

n = number of moles  

R = gas constant = 0.08205 l.atm / mol K  

T = temperature, Kelvin  

Gas Ne with :

moles : 0.019135

volume : 878.3 ml = 0.8783 L

Pressure : 0.946 atm

Plug in gas ideal equation :

Which equation agrees with the ideal gas law  

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Which law relates to the ideal gas law  

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i think so it’s will be b yes i believe its

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